pKa Table of Common acids

The pKa value of a molecule describes its acidity. A pKa table simplifies pKa values. It determines an acid’s strength by how firmly a proton is retained by a Bronsted acid. The lower the pKa value, the more powerful the acid and its capacity to transfer protons. define a molecule’s acidity.

pKa Table
pKa Table

What is pKa?

pKa is the negative base-10 logarithm of a solution’s acid dissociation constant (Ka).

Both pKa and Ka provide information in certain ways, however the Ka value is a tiny decimal number that is easy to deal with, whereas Ka contains exponents and employs scientific notation.

Relationship Between pKa and Ka

  • pKa = -log10Ka
  • Ka = 10-pKa

How to use a pKa Table

  • pKa values have been recorded for a vast variety of compounds and are mainly connected to the molecule’s most acidic functional group. A pKa table simplifies pKa values.
  • A low pKa value (for example, -10) implies a strong acid. A high pKa value (for example, 50) implies a weak acid.
  • A conjugate acid and a conjugate base are formed when an acid and a base swap a bond to H.
  • Acid-base reactions are always represented as equilibria, which occur in either a forward or backward direction. A stronger acid and a stronger base generate a weaker acid and a weaker base, which is the preferred direction for an acid-base interaction.
  • By comparing the pKa of the acid and the conjugate acid, one may determine which way is preferred. The formation of the weaker acid (molecule with higher pKa) will be preferred.
  • These principles can also be applied to other reactions (for example, substitution reactions).

pKa Table for common acids

AcidFormulapKa
Acetic acidCH3COOH4.76
Formic acidHCOOH3.75
PhenolC6H5OH10
Hydrofluoric acidHF3.20
Nitrous acidHNO23.25
Hydrocyanic acidHCN9.3
Phosphoric acidH3PO42.16
AlkaneCH450
AlkyneCH☰CH25
Oxalic acidH2C2O41.2
Trifluoro acetic acidCF3COOH0.52
Nitric acidHNO3-1.4
WaterH2O14
Sulfuric acidH2SO4-3
Hydrogen sulphideH2S7.05
Hydrochloric acidHCl-7
Carbonic acidH2CO36.35
Perchloric acidHClO4-10
Hydroiodic acidHI-9.5
Hydronium ionH3O+-1.74
AmineNH335
Boric acidH3BO39.15
Cyanic acidHOCN3.46

pKa Table Organic Chemistry

Most organic acids have pKa values between 5-60. While it is difficult to determine the pKa of every organic molecule, understanding the pKa (and acidity) based on the functional groups involved is extremely important because the same functional groups typically have comparable pKa.

Table here shows the approximate ranges of pKa values for seven key functional groups, which may be used to predict and understand the acidity of any organic molecule.

Functional GrouppKa
Carboxylic acid∼5
Alcohol∼16
Aldehyde/ Ketone∼16 -20
Alkyne∼25
Amine∼35-40
Alkene∼45
Alkane ∼>50

How to Predict the Position of Equilibrium in Organic Acid-Base Reactions Using values in pKa table 

To estimate the location of equilibrium in the following reaction, we must first decide what will be the acid and what will be the base on both the left and right. The conjugate base is formed when the base accepts the acidic proton. This means that the hydroxide ion serves as a base and acetic acid serves as an acid. In the opposite reaction, however, water acts as an acid and acetic ion acts as a base. The acetic ion is an acetic acid conjugate base, while the hydroxide is a water conjugate base.

When we compare the pKa values of these acids (acetic acid and water), we observe that the left side is 4.75 and the right side is 15.7. Because the equilibrium favors the weaker acid, the acid with the higher pKa value will win. This will be water with a higher pKa value in this situation. This signifies that the equilibrium is to the right.

PKa table of acid with conjugate bases [Image source: chemistryscore.com]

References

  • https://chemistryscore.com/use-pka-table/
  • https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Organic_Chemistry_I_(Cortes)/11%3A_Bronsted_Acid-Base_Chemistry/11.04%3A_pKa_Table
  • https://byjus.com/chemistry/pka/#:~:text=FAQs-,Definition%20of%20pKa,ability%20to%20donate%20its%20protons.
  • Atkins, Peter; de Paula, Julio (2006). Physical Chemistry. Oxford. ISBN 978-0198700722.
  • Denbigh, K. (1981). “Chapter 4.” The Principles of Chemical Equilibrium (4th ed.). Cambridge: Cambridge University Press. ISBN 978-0-521-28150-8.
  • https://sciencenotes.org/what-is-pka-in-chemistry-acid-dissociation-constant/
  • https://www.masterorganicchemistry.com/2010/09/29/how-to-use-a-pka-table/#five
  • https://organicchemistrydata.org/hansreich/resources/pka/

About Author

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Jyoti Bashyal

Jyoti Bashyal, a graduate of the Central Department of Chemistry, is an avid explorer of the molecular realm. Fueled by her fascination with chemical reactions and natural compounds, she navigates her field's complexities with precision and passion. Outside the lab, Jyoti is dedicated to making science accessible to all. She aspires to deepen audiences' understanding of the wonders of various scientific subjects and their impact on the world by sharing them with a wide range of readers through her writing.

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